If I contain 1.7 moles of gas in a container with a volume of 133 liters and at a temperature of 393 K, what is the pressure inside the container in mmHg?

The first step is always to figure out which formula you are going to use. Since you are given the moles, volume, temperature, and are asked for pressure, you will obviously be using the ideal gas law.

P = ?

V = 133 L

n = 1.7

R = 8.314

T = 393K

P = 41.76378496 kPa

Last step is to convert to mmHg

= 41.76378496 kPa  x  

= 313.2541482

= 3.1 x 10² mmHg

here's the link to your question!

explanation:

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2