What is the pressure in $m m \cdot H g$ $mmHg$ if a $4.0 \cdot g$ $4.0g$ mass of oxygen gas at $303 \cdot K$ $303K$ was confined to a container whose volume of $3000 \cdot m L$ $3000mL$ ?

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What is the pressure in $m m \cdot H g$ $mmHg$ if a $4.0 \cdot g$ $4.0g$ mass of oxygen gas at $303 \cdot K$ $303K$ was confined to a container whose volume of $3000 \cdot m L$ $3000mL$ ?

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Answer 1 · 2017-06-28T20:51:40

$P=1.04*atm.......$

Explanation:

We use the Ideal Gas Equation, to give.....

$P=(nRT)/V=((4.00*g)/(32.00*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx303*K)/(3000*mLxx10^-3*L*mL^-1)$

$=1.04*atm$

Now had the pressure been UNDER $1*atm$ I could use the relationship $1*atm-=760*mm*Hg$ ; i.e. an atmosphere will support a column of mercury that is so high. You do not measure a pressure that is greater than $1*atm$ in $mm*Hg$ . Whoever set this problem was ignorant.........

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What is the pressure in $m m \cdot H g$ $mmHg$ if a $4.0 \cdot g$ $4.0g$ mass of oxygen gas at $303 \cdot K$ $303K$ was confined to a container whose volume of $3000 \cdot m L$ $3000mL$ ?

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What is the pressure in mm*Hgmm⋅Hgmm*Hg if a 4.0*g4.0⋅g4.0*g mass of oxygen gas at 303*K303⋅K303*K was confined to a container whose volume of 3000*mL3000⋅mL3000*mL?

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What is the pressure in $m m \cdot H g$ $mmHg$ if a $4.0 \cdot g$ $4.0g$ mass of oxygen gas at $303 \cdot K$ $303K$ was confined to a container whose volume of $3000 \cdot m L$ $3000mL$ ?