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timofeeve [1]
2 years ago
11

What is the mass of bismuth carbonate (597.99 g/mol) that decomposes to release 50.0ml of carbon dioxide gas at stp? 0.000445 g

0.00400 g 0.445 g 1.33 g 4.00 g?
Chemistry
1 answer:
REY [17]2 years ago
5 0

The mass of bismuth carbonate that decomposed is 0.445 g


calculation

write the equation for reaction


that is Bi2(CO3)3 → Bi2O3 +3 CO2



find the moles of of CO2 formed


At STP 1 mole of a gas = 22.4 L

what about 50 Ml


convert the Ml to Liters = 50/1000= 0.05 L


moles of CO2 formed is therefore= 1 mole x 0.05 L/22.4 l =2.232 x10^-3 moles


by use of reacting ratio between Bi(CO3)3 to CO2 which is 1:3 the moles of Bi(CO3)3 is = 2.232 x10^-3 x1/3= 0.744 x10^-4 moles of Bi(CO3)3


mass of Bi(CO3)3 = molar mass x number of moles


mass= 0.744 x10^-4 moles x 597.99 g/mol = 0.445 grams


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The molar mass of a gas if a flask with a volume of 3. 16 L contains 9. 33 grams of the gas at 32. 0°C and 1. 00 atm is  1.17g/mol

Calculation ,

In this question we have to fist find the number of moles of gas by using ideal gas equation and from the help of number of moles we can determine molar mass.

According to ideal gas equation which is also known as ideal law ,

PV = nRT                ...( i )

where P is the pressure of the gas = 1 atm

V is the volume of the gas in the flask with volume =  3. 16 L

R is the universal gas constant = 0.082 atm L/K mol

T is the temperature = 32. 0°C = 32 + 273 = 305 K

n is the number of moles = ?

Putting the value of Pressure P , volume V , temperature T , number of moles n and universal gas constant R in the equation (i) we get ,

1 atm ×3. 16 L = n× 0.082 atm L/K mol ×305 K

n = 1 atm ×3. 16 L / 0.082 atm L/K mol × 305 K = 0.126 mole

number of mole of a gas  = 0.126 mole = given mass/ molar mass

molar mass  = number of moles × Given mass =  0.126 × 9. 33 = 1.17g/mol

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