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m_a_m_a [10]
3 years ago
8

354.5 g of chlorine gas is held with a fixed volume of 70.0 L. What is the pressure of the gas in atmospheres if it’s temperatur

e is 30.0 C
Chemistry
1 answer:
zaharov [31]3 years ago
7 0

Answer: The pressure of the gas in atmospheres is 1.76

Explanation:

According to ideal gas equation:

PV=nRT

P = pressure of gas = ?

V = Volume of gas = 70.0 L

n = number of moles = \frac{\text {given mass}}{\text {Molar mass}}=\frac{354.5g}{71g/mol}=5moles

R = gas constant =0.0821Latm/Kmol

T =temperature =30.0^0C=(30.0+273)K=300.0K

P=\frac{nRT}{V}

P=\frac{5\times 0.0821Latm/K mol\times 300K}{70.0L}=1.76

Thus the pressure of the gas in atmospheres is 1.76

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This question is an incomplete question, here is a complete question.

Perform the following calculation. Report the answer using the proper number of significant figures.

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Explanation :

Significant figures : The figures in a number which express the value -the magnitude of a quantity to a specific degree of accuracy is known as significant digits.

The rule apply for the multiplication and division is :

The least number of significant figures in any number of the problem determines the number of significant figures in the answer.

The rule apply for the addition and subtraction is :

The least precise number present after the decimal point determines the number of significant figures in the answer.

The given expression is,

\frac{1.012\times 10^{-3}J}{(0.025456g)\times (298.3682-298.3567)K}

\frac{1.012\times 10^{-3}J}{(0.025456g)\times (0.0115)K}

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Answer:

See explaination

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