To solve this we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:
P1V1 =P2V2
P2 = P1V1/V2
P2 = 740mmhg x 19 mL / 30 mL
P2 = 468.67 mmHg = 0.62 atm
Answer: The new pressure will be 0.616 atm
Explanation:
To calculate the new pressure, we use the equation given by Boyle's law. This law states that pressure is directly proportional to the volume of the gas at constant temperature.
The equation given by this law is:
[tex]P_1V_1=P_2V_2[/tex]
where,
[tex]P_1\text{ and }V_1[/tex] are initial pressure and volume.
[tex]P_2\text{ and }V_2[/tex] are final pressure and volume.
We are given:
[tex]P_1=740mmHg\\V_1=19mL\\P_2=?mmHg\\V_2=30mL[/tex]
Putting values in above equation, we get:
[tex]740mmHg\times 19mL=P_2\times 30mL\\\\P_2=468.66mmHg[/tex]
Converting this into atmospheres, we use the conversion factor:
1 atm = 760 mmHg
Now, converting the given quantity, we get:
[tex]\Rightarrow \frac{1atm}{760mmHg}\times 468.66mmHg=0.616atm[/tex]
Hence, the new pressure will be 0.616 atm.
