A sample of 3.00 g of SO21g2 originally in a 5.00-L vessel at
21 ...

Question

A sample of 3.00 g of SO21g2 originally in a 5.00-L vessel at
21 °C is transferred to a 10.0-L vessel at 26 °C. A sample of
2.35 g of N21g2 originally in a 2.50-L vessel at 20 °C is transferred
to this same 10.0-L vessel. (a) What is the partial
pressure of SO21g2 in the larger container?

Accepted Answer

Hi everyone simmer for 4.5 L cylinder which contained 4. g of hydrogen cyanide gas At 35°C. And the gas cylinder is emptied into a 7.65 L cylinder At 27°C which contains 5.54 g of national gas. They were asking the partial pressure of hydrogen cyanide and the 7.65 liter cylinder. We need to first find the moles of hydrogen cyanide. Then we can play into the ideal gas law. Find the partial pressure of hydrogen cyanide, 4.67 g of hydrogen cyanide. And in one mall of hydro cyanide we have the molar mass And this is 1.008 g Past 12.011 g Plus 14.007 g. Give us 27.026 gramps. So this will give us 0.173 malls of hydro cyanide. So now we can plug this into the ideal gas law which is B people's N. R. T. And we can rearrange this to solve for pete. Would you be N. R. T. About five P. And the pressure is what we're looking for. The number of moles, 0.173. That our value 0.08206. There are some atmosphere to buy malls Calvin. The temperature is 27°C and we need to have the temperature in kelvin, We need to add 273 115. Let's give us 300 15 kelvin in the volume Is 7.65 L. So now we plug in these bags are going to get peak Equals 0. malls Time 0.08 to our sex. Later Sounds atmosphere. What about malls, Calvin times 300 . Kelvin Divide by 7.65 Leaders for the pressure. Gonna get 0.55 seven atmosphere. Thanks for watching my video. And I hope it was helpful.

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