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2 years ago

How many grams of NH4OH are present in 37.0 grams of 6.00 M NH4OH which has a density of 0.960 g/mL?

Chemistry

1 answer:

inn [45]2 years ago

6 0

Answer:

The mass of NH₄OH present in the solution is 8.085 g

Explanation:

Given;

molarity of NH₄OH = 6 M

density of NH₄OH = 0.960 g/mL

mass of NH₄OH = 37.0 grams

volume of NH₄OH = mass /density

= 37/0.96

= 38.54 mL

molarity = moles of solute / Liters of solution

moles of solute = molarity x Liters of solution

moles of solute = 6 x 38.54 x 10⁻³

moles of solute = 0.231 moles

Reacting mass = number of moles x molecular mass

Molecular mass of NH₄OH = 35 g/mol

Reacting mass = 0.231 mol x 35 g/mol

Reacting mass = 8.085 g

Therefore, the mass of NH₄OH present in the solution is 8.085 g

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The chemical reaction that causes chromium to corrode in air is given by 4Cr+3O2→2Cr2O3 in which at 298 K ΔH∘rxn = −2256 kJ ΔS∘r

MAVERICK [17]

Answer:

-2092 kJ

Explanation:

Let's consider the chemical reaction that causes chromium to corrode in air.

4 Cr + 3 O₂ → 2 Cr₂O₃

We can calculate the standard Gibbs free energy (ΔG°) using the following expression.

ΔG° = ΔH° - T × ΔS°

where,

ΔH°: standard enthalpy of the reaction

T: absolute temperature

ΔS°: standard entropy of the reaction

ΔG° = -2256 kJ - 298 K × (-0.5491 kJ/K)

ΔG° = -2092 kJ

5 0

2 years ago

Read 2 more answers

What is the final pressure (expressed in atm) of a 3.05 l system initially at 724 mm hg and 298 k, that is compressed to a final

krok68 [10]

<u>Answer:</u>

P2 = 778.05 mm Hg = 1.02 atm

<u>Explanation:</u>

We are to find the final pressure (expressed in atm) of a 3.05 liter system initially at 724 mm hg and 298 K which is compressed to a final volume of 2.60 liter at 273 K.

For this, we would use the equation:

$\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}$

where P1 = 724 mm hg

V1 = 3.05 L

T1 = 298 K

P2 = ?

V2 = 2.6 L

T2 = 173 K

Substituting the given values in the equation to get:

$\frac{(724)(3.05)}{298} =\frac{P_2(2.6)}{173}$

P2 = 778.05 mm Hg = 1.02 atm

7 0

2 years ago

Write the balanced chemical equation for the reaction shown.

son4ous [18]

Explanation:

Carbon black sphere

Nitrogen blue sphere

Chlorine green sphere

Hydrogen white sphere

Reactants:

three molecules that contain one black sphere and four white spheres

3CH₄

three molecules that contain two blue spheres and four green spheres:

3N₂Cl₄

Products:

three molecules that contain one black sphere and four green spheres:

3CCl₄

three molecules that contain two blue spheres:

3N₂

six molecules that contain two white spheres

6H₂

The reaction proper:

3CH₄ + 3N₂Cl₄ → 3CCl₄ + 3N₂ + 6H₂

Learn more:

Chemical reactions brainly.com/question/4216541

#learnwithBrainly

7 0

2 years ago

The combustion of one mole of liquid ethanol, CH3CH2OH, produces 1367 kJ of heat. Calculate how much heat is produced when 235.0

deff fn [24]

Answer:- 6984 kJ of heat is produced.

Solution:- From given information, 1367 kJ of heat is produced by the combustion of 1 mole of ethanol. We are asked to calculate the heat produced by the combustion of 235.0 g of ethanol.

Let's convert given grams to moles and multiply by the heat produced by one mole of ethanol to get the total heat produced. Molar mass of ethanol is 46 grams per mole. The set will be:

$235.0g(\frac{1mole}{46g})(\frac{1367 kJ}{1mole})$

= 6984 kJ

So, 6984 kJ of heat is produced by the combustion of 235.0 g of liquid ethanol.

6 0

2 years ago

Which substance absorbs 58.16 kJ of energy when 3.11 mol vaporizes? a)CH4 b)H2S c)CO2 d)NaCl

schepotkina [342]

Answer:

$H_2S$

Explanation:

Given the amount of heat absorbed and the amount of substance in moles, we may calculate the heat of vaporization. Heat of vaporization is defined as the amount of heat per 1 mole of substance required to evaporate that specific substance.

Based on the value of heat of vaporization, we will identify the substance. Firstly, let's calculate the heat of vaporization:

$\Delta H^o = \frac{58.16 kJ}{3.11 mol} = 18.7 kJ/mol$

Secondly, let's use any table for heat of vaporization values for substances. We identify that the heat of vaporization of $H_2S$ is 18.7 kJ/mol

8 0

2 years ago