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1 year ago

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Ammonia (nh3(g), hf = –46.19 kj/mol) reacts with hydrogen chloride (hcl(g), hf = –92.30 kj/mol) to form ammonium chloride (nh4cl

(s), hf = –314.4 kj/mol) according to this equation: nh3(g) + hcl(g) nh4cl(s) what is hrxn for this reaction?

2 answers:

Ainat [17]1 year ago

9 0

Answer:-175.9

Explanation:

trust

steposvetlana [31]1 year ago

8 0

Answer: The $\Delta H_{rxn}$ for the given chemical reaction is -175.51 kJ/mol

Explanation: Enthalpy change of the reaction is defined as the amount of heat released or absorbed in a given chemical reaction.

Mathematically,

$\Delta H_{rxn}=\Delta H_f_{(products)}-\Delta H_f_{(reactants)}$

We are given a chemical reaction. The reaction follows:

$NH_3(g)+HCl(g)\rightarrow NH_4Cl(s)$

$H_f_{(NH_3)}=-46.19kJ/mol$

$H_f_{(HCl)}=-92.30kJ/mol$

$H_f_{(NH_4Cl)}=-314.4kJ/mol$

Enthalpy change for the reaction of he given chemical reaction is given by:

$\Delta H_{rxn}=H_f_{(NH_4Cl)}-(H_f_{(NH_3)}+H_f_{(HCl)})$

Putting the values in above equation, we get

$\Delta H_{rxn}=-314.4-(-92.30-46.19)kJ/mol$

$\Delta H_{rxn}=-175.51kJ/mol$

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For scuba dives below 150 ft, helium is often used to replace nitrogen in the scuba tank. If 15.2 g of He(g) and 30.6 g of O2(g)

abruzzese [7]

Answer:

see explanation below

Explanation:

To do this exercise, we need to use the following expression:

P = nRT/V

This is the equation for an ideal gas. so, we have the temperature of 22 °C, R is the gas constant which is 0.082 L atm / mol K, V is the volume in this case, 5 L, and n is the moles, which we do not have, but we can calculate it.

For the case of the oxygen (AW = 16 g/mol):

n = 30.6 / 32 = 0.956 moles

For the case of helium (AW = 4 g/mol)_

n = 15.2 / 4 = 3.8 moles

Now that we have the moles, let's calculate the pressures:

P1 = 0.956 * 0.082 * 295 / 5

P1 = 4.63 atm

P2 = 3.8 * 0.082 * 295 / 5

P2 = 18.38 atm

Finally the total pressure:

Pt = 4.63 + 18.38

Pt = 23.01 atm

7 0

2 years ago

Ethyl butyrate, CH3CH2CH2CO2CH2CH3, is an artificial fruit flavor commonly used in the food industry for such flavors as orange

SIZIF [17.4K]

Answer:

A. 10.0 grams of ethyl butyrate would be synthesized.

B. 57.5% was the percent yield.

C. 7.80 grams of ethyl butyrate would be produced from 7.60 g of butanoic acid.

Explanation:

$CH_3CH_2CH_2CO_2H(l)+CH_2CH_3OH(l)+H^+\rightarrow CH_3CH_2CH_2CO_2CH_2CH_3(l)+H_2O(l)$

A

Moles of butanoic acid = $\frac{7.60 g}{88 g/mol}=0.08636 mol$

According to reaction ,1 mole of butanoic acid gives 1 mol of ethyl butyrate,then 0.08636 mol of butanoic acid will give :

$\frac{1}{1}\times 0.08636 mol=0.08636 mol$ of ethyl butyrate

Mass of 0.08636 moles of ethyl butyrate =

0.08636 mol × 116 g/mol = 10.0 g

Theoretical yield = 10.0 g

Experimental yield = ?

Percentage yield of the reaction = 100%

$Yield\%=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

$100\%=\frac{\text{Experimental yield}}{10.0 g}\times 100$

Experimental yield = 10.0 g

10.0 grams of ethyl butyrate would be synthesized.

B

Theoretical yield of ethyl butyrate = 10.0 g

Experimental yield ethyl butyrate = 5.75 g

Percentage yield of the reaction = ?

$Yield\%=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

$=\frac{5.75 g}{10.0 g}\times 100=57.5\%$

57.5% was the percent yield.

C

Moles of butanoic acid = $\frac{7.60 g}{88 g/mol}=0.08636 mol$

According to reaction ,1 mole of butanoic acid gives 1 mol of ethyl butyrate,then 0.08636 mol of butanoic acid will give :

$\frac{1}{1}\times 0.08636 mol=0.08636 mol$ of ethyl butyrate

Mass of 0.08636 moles of ethyl butyrate =

0.08636 mol × 116 g/mol = 10.0 g

Theoretical yield = 10.0 g

Experimental yield = ?

Percentage yield of the reaction = 78.0%

$Yield\%=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

$78.0\%=\frac{\text{Experimental yield}}{10.0 g}\times 100$

Experimental yield = 7.80 g

7.80 grams of ethyl butyrate would be produced from 7.60 g of butanoic acid.

8 0

1 year ago

30. how many grams of boric acid, b(oh)3 (fm 61.83), should be used to make 2.00 l of 0.050 0 m solution? what kind of fl ask is

grigory [225]

Answer:

Mass = 6.183 g

Solution:

Step 1: Calculate number of moles of Boric acid using following formula,

Molarity = Moles ÷ Volume

Solving for Moles,

Moles = Molarity × Volume

Putting Values,

Moles = 0.05 mol.L⁻¹ × 2.0 L

Moles = 0.1 mol

Step 2: Calculate Mass of Boric Acid using following formula,

Moles = Mass ÷ M.mass

Solving for Mass,

Mass = Moles × M.mass

Putting values,

Mass = 0.1 mol × 61.83 g.mol⁻¹

Mass = 6.183 g

Flask used to prepare this solution is called as Volumetric flask. Take 2 L volumetric flask, add 6.183 g of Boric acid and fill it to the mark with distilled water.

7 0

2 years ago

It requires 0.0780L of a 0.12 M HCl solution to completely neutralize 0.0280L of an unknown LiOH solution. What is the concentra

kari74 [83]

Answer:

C₂ = 0.334 M

Explanation:

Given data:

Volume of HCl = 0.0780 L

Concentration of HCl = 0.12 M

Volume of LiOH = 0.0280 L

Concentration of LiOH = ?

Solution:

Formula:

C₁V₁ = C₂V₂

C₁ = Concentration of HCl

V₁ = Volume of HCl

C₂ = Concentration of LiOH

V₂ = Volume of LiOH

Now we will put the values in formula.

C₁V₁ = C₂V₂

0.12 M × 0.0780 L = C₂ × 0.0280 L

0.00936 M.L = C₂ × 0.0280 L

C₂ = 0.00936 M.L/0.0280 L

C₂ = 0.334 M

4 0

1 year ago

Perform the following conversion: 6.1 × 103 K (the surface temperature of the Sun) to °F and °C. Pay attention to the number of

Keith_Richards [23]

Answer:

$\°C=5.8x10^3\°C$

$\°F=1.1x10^4\°F$

Explanation:

Hello,

In this case, for the calculation of the temperature in degree Celsius we subtract 273.15 to the given temperature in kelvins:

$\°C=6100-273.15\\\\\°C=5.8x10^3\°C$

Next, by applying the following equation we compute it in degree Fahrenheit:

$\°F=(5.8x10^{3}*9/5) + 32\\\\\°F=1.1x10^4\°F$

Clearly, since the initial unit has two significant figures the computed units also show two significant figures.

Regards.

5 0

1 year ago