a gas at 701 mmhg and 32 °c occupies a volume of 6.63 l. calculate its volume at stp. be sure your answer…

Explanation:

Step1: Convert initial pressure to atm

The initial pressure $P_1 = 701\ mmHg$. Since $1\ atm=760\ mmHg$, then $P_1=\frac{701}{760}\ atm\approx0.922\ atm$. The initial temperature $T_1=(32 + 273.15)\ K=305.15\ K$, the initial volume $V_1 = 6.63\ L$. At STP, $P_2 = 1\ atm$ and $T_2=273.15\ K$. $P_1=\frac{701}{760}\ atm\approx0.922\ atm$

Step2: Use the combined - gas law

The combined - gas law is $\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$. We want to solve for $V_2$. Rearranging the formula gives $V_2=\frac{P_1V_1T_2}{T_1P_2}$. $V_2=\frac{0.922\ atm\times6.63\ L\times273.15\ K}{305.15\ K\times1\ atm}$

Step3: Calculate the final volume

$V_2=\frac{0.922\times6.63\times273.15}{305.15}\ L$ $V_2=\frac{0.922\times6.63\times273.15}{305.15}\approx5.52\ L$

Answer:

$5.52\ L$