Chemistry help im desperate

A sample of helium gas has a volume of 4.50L at a pressure of 835 mmHg and a temperature of 20 *C

p1=?? atm.

1. What is the pressure of the gas in atm when the volume and temperature of the gas sample are changed to 1800L and 330 * C , respectively?

2.What is the pressure of the gas in atm when the volume and temperature of the gas sample are changed to 2.40 L and 15,8 C respectively?

3.What is the pressure of the gas in atm when the volume and temperature of the gas sample are changed to 14.0L and 48 *C?

A sample of helium gas has a volume of 4.50L at a pressure of 835 mmHg and a temperature of 20 *C

1 atm = 760 mm Hg

p1= 835/760 atm =

Use the following equation,
(P1 * V1) ÷ T1 = (P2 * V2) ÷ T2
Pressure in atm
Volume in liters
Temperature in ˚K = ˚C + 273

(835/760 * 4.50) ÷ (293) = (P2 * V2) ÷ T2


1. What is the pressure of the gas in atm when the volume and temperature of the gas sample are changed to 1800L and 330 * C + 273 = 603˚ , respectively?
(835/760 * 4.50) ÷ (293) = (P2 * 1800) ÷ 603
Solve for P

2.What is the pressure of the gas in atm when the volume and temperature of the gas sample are changed to 2.40 L and 15.8 C + 273 = respectively?

(835/760 * 4.50) ÷ (293) = (P2 * 2.40) ÷ 288.8

3.What is the pressure of the gas in atm when the volume and temperature of the gas sample are changed to 14.0L and 48 + 273
Same #2
(835/760 * 4.50) ÷ (293) =

P1*V1/T1=P2*V2/T2