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2 years ago

What mass of carbon dioxide gas occupies a volume of 81.3L at 204 kPa and a temperature of 95.0°C?

Chemistry

1 answer:

alexandr1967 [171]2 years ago

5 0

Answer:

236.9g

Explanation:

Given parameters:

Volume of gas = 81.3L

Pressure of gas = 204kPa

temperature of gas = 95°C

Unknown:

Mass of carbondioxide gas = ?

Solution:

To solve this problem, the ideal gas law will be well suited. The ideal gas law is a fusion of Boyle's law, Charles's law and Avogadro's law.

Mathematically, it is expressed as;

PV = nRT

the unknown here is n which is the number of moles;

P is the pressure, V is the volume, R is the gas constant and T is the temperature.

convert pressure into atm

101.325KPa = 1atm

204 kPa = $\frac{204}{101.325}$ = 2atm

Convert temperature to Kelvin; 95 + 273 = 368K

2 x 81.3 = n x 0.082 x 368

n = $\frac{2 x 81.3}{0.082 x 368}$ = 5.38moles

Since the unknown is mass;

Mass = number of moles x molar mass

Molar mass of carbon dioxide = 12 + 2(16) = 44g/mol

Mass = 5.38 x 44 = 236.9g

You might be interested in

Which polyatomic ion is found in the compound represented by the formula NaHCO3?

olga nikolaevna [1]

Answer is (2) - hydrogen carbonate

Explanation:

NaHCO₃ is an ionic compound which is made from Na⁺ and HCO₃⁻ ions. The decomposition is

NaHCO₃ → Na⁺ + HCO₃⁻

Among the resulted ions, Na⁺ is a monatomic ion while HCO₃⁻ is a polyatomic ion.

Polyatomic ions mean ions which are made of two or more different atoms.

HCO₃⁻ is made from 3 atoms as H, C and O. The name of HCO₃⁻ ion is bicarbonate or hydrogen carbonate.

8 0

2 years ago

How many grams of BaCl2 are formed when 35.00 mL of 0.00237 M Ba(OH)2 reacts with excess Cl2 gas? 2 Ba(OH)2(aq) + 2 Cl2(g) → Ba(

Vesna [10]

Answer:

0.0071g

Explanation:

From the question, we know that the molarity of the BaCl2 is 0.00237M. This means there are 0.00237 moles in 1dm^3 or 1000cm^3 of solution.

We also know that 35ml of the BaCl2 reacted. Here, we need to calculate the number of moles in 35.7ml of BaCl2.

This is calculated as follows;

0.00237moles are in 1000cm^3

Thus x moles will be present in 35ml ( we should note that cm^3 is same as ml)

X = (0.00237 × 35) ÷ 1000 = 0.00008295 moles.

From the reaction equation, we can see that 2 moles of BaCl2 yielded 1 mole of Ba(OH)2.

This means 0.00008295mole of BaCl2 will yield 0.00008295 ÷ 2 = 0.000041475 moles of Ba(OH)2.

To calculate the mass of Ba(OH)2 formed, we simple multiply the number of moles yielded by the molar mass of Ba(OH)2.

Molar mass of Ba(OH)2 = 137 + 2(17)

= 171g/mol

Mass = 171 × 0.000041475 = 0.007092225g

3 0

2 years ago

What is the ph of a solution of 0.400 m k2hpo4, potassium hydrogen phosphate?

dusya [7]

When we can get Pka for K2HPO4 =6.86 so we can determine the Ka :

when Pka = - ㏒ Ka

6.86 = -㏒ Ka

∴Ka = 1.38 x 10^-7

by using ICE table:

H2PO4- → H+ + HPO4
initial 0.4 m 0 0

change -X +X +X

Equ (0.4-X) X X

when Ka = [H+][HPO4] / [H2PO4-]

by substitution:

1.38 X 10^-7 = X^2 / (0.4-X) by solving for X

∴X = 2.3x 10^-4

∴[H+] = X = 2.3 x 10^-4

∴PH = -㏒[H+]

= -㏒ (2.3 x 10^-4)
∴PH = 3.6

3 0

2 years ago

If 6.00 g of the unknown compound contained 0.200 mol of C and 0.400 mol of H, how many moles of oxygen, O, were in the sample?

Arada [10]

Convert moles to mass.

mass C = 0.2 mol * 12 g / mol = 2.4 g

mass H = 0.4 mol * 1 g / mol = 0.4 g

So mass left for O = 6 g – (2.4 g + 0.4 g) = 3.2 g

Calculating for moles O given mass:

moles O = 3.2 g / (16 g / mol) = 0.2 moles

Answer:

0.2 moles O