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omeli [17]
3 years ago
9

A sample of hydrogen gas at a pressure of 977 mm Hg and a temperature of 32 °C, occupies a volume of 11.3 liters. If the gas is

cooled at constant pressure to a temperature of -5 °C, the volume of the gas sample will be L.
Chemistry
1 answer:
IrinaK [193]3 years ago
6 0

Answer : The volume of gas sample will be, 9.93 L

Explanation :

Charles' Law : It states that volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles of gas.

Mathematically,

\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1\text{ and }T_1 are the initial volume and temperature of the gas.

V_2\text{ and }T_2 are the final volume and temperature of the gas.

We are given:

V_1=11.3L\\T_1=32^oC=(32+273)K=305K\\V_2=?\\T_2=-5^oC=(-5+273)K=268K

Now put all the given values in above equation, we get:

\frac{11.3L}{305K}=\frac{V_2}{268K}\\\\V_2=9.93L

Therefore, the volume of gas sample will be, 9.93 L

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5.499 g of NaCl is formed if 5.00 g of pure Na2CO3 is treated with HCl solution

The equation of the reaction is;

2HCl  +  Na2CO3 ----->2NaCl + H2O + CO2

Molar mass of Na2CO3 = 2(23) + 12 + 3(16) = 46 + 12 +48 = 106 g/mol

The number of moles of Na2CO3 in 5.00 g of pure Na2CO3 = 5g/106 g/mol

= 0.047 moles

From the reaction equation;

1 mole of Na2CO3  yields 2 moles of NaCl

0.047 moles of Na2CO3  yields 0.047 × 2/1 = 0.094 moles

Molar mass of NaCl = 23 + 35.5 = 58.5 g/mol

Mass of NaCl = 0.094 moles × 58.5 g/mol

Mass of NaCl =  5.499 g of NaCl

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