15.0 g of carbon dioxide gas is stored in a cylinder (a malfunctioned fire extinguisher) with a volume of 10.0 L. A pressure gauge shows the pressure to be 3.00 atm. Determine the temperature of the gas in degrees celsius. R=0.0821 L·atm/(mol·K)

Consider the following balanced equation. 2 Sb (s)  +   3 H2O (g)    →   Sb2O3 (s)   +   3 H2 (g) 5.0 L of H2O gas, with a pressure of 1.29 atm and a temperature of 96.7 °C reacted. How many mol of Sb2O3 were formed? Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, liters = L, atmospheres = atm   What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank.     Calculate the mol of H2O reacted (enter value only, with proper s.f.).  mol   Use the three blanks to enter the number, unit, and substance (in this order) that appears in…

A sample of 250. ml of NH3 gas at 22 celcius is heated at constant pressure until it fills a volume of 500. ml. What is the new temperature in Celcius?

A flask of ammonia is connected to a flask of an unknown acid HX by a 1.12 m glass tube (where "X" represents a halogen). As the two gases diffuse down the tube, a white ring of NH₂X forms 76.7 cm from the ammonia flask. Identify element X (Name or symbol).

Consider the reaction below which was carried out at 200.0 K to produce liquid ammonia: N2(8) + 3H,(g) 2NH3() Suppose 37.3 g of N2 gas is mixed with 37.3 g of H2 gas. What is the volume (in units of liters) of gas remaining after the reaction is completed? The remaining gas was measured to have a temperature of 200.0 K and a pressure of 760.0 mmHg? molar mass of N2= 28.013 g/mol molar mass of H2 = 2.0158 g/mol. %3D Recall: Vo (1/P) (at constant Tand n) VaT (at constant P and n) Van (at constant Tand P) PV = nRT rate of effusion ox 1 atm 760 torr 760 mmHg %3D %3D R=8.31446 J K-1.r mol-1 R= 0.0820573L atm K-1. mol-1 %3D

There is 17.0 g of carbon dioxide gas stored in a cylinder with a volume of 12.0. A pressure gauge shows the pressure to be 2.00 atm. R=0.0821 L·atm/(mol·K) In degrees Celsius, determine the temperature of the gas.

For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point of −33.°C.Suppose the temperature of a sample of ammonia gas is lowered from 10.0°C⁢ to −25.0°C, and at the same time the pressure is changed. If the initial pressure was 6.6atm and the volume increased by 40.0%, what is the final pressure? Round your answer to the correct number of significant digits.

Consider the following balanced equation. 2 Sb (s)  +   3 H2O (g)    →   Sb2O3 (s)   +   3 H2 (g) 5.0 L of H2O gas, with a pressure of 1.29 atm and a temperature of 96.7 °C reacted. How many mol of Sb2O3 were formed? Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, liters = L, atmospheres = atm   What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank.     Calculate the mol of H2O reacted (enter value only, with proper s.f.).  mol   Use the three blanks to enter the number, unit, and substance (in this order) that appears in…

A flask of ammonia is connected to a flask of an unknown acid HX by a 1.14  m glass tube (where "X" represents a halogen). As the two gases diffuse down the tube, a white ring of NH4X forms 78.1  cm from the ammonia flask. Identify element X (Name or symbol).

The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed   rms speed= the square root of 3RT/M   where R=8.314 J/(mol⋅K) and ℳ is molar mass in kilograms per mole. Note that a joule is the same as a kilogram‑meter squared per second squared (kg·m2/s2). What is the rms speed of N2 molecules at 357 K?   What is the rms speed of He atoms at 357 K?