We can determine the pressure of a mixture of HCl (g) and `NH_(3(g))` by using the formula, total pressure of the mixture, `P = P_HCl + P_NH_3`
How is it applicable to calculate the pressure of a gas collected over water at a known temperature?

We can determine the pressure of a mixture of HCl (g) and NH_(3(g)) by using the formula, total pressure of the mixture, P = P_HCl + P_NH_3 Explain the law behind this.

We can determine the pressure of a mixture of HCl (g) and NH_(3(g)) by using the formula, total pressure of the mixture, P = P_HCl + P_NH_3 Analyse the statement and write your opinion.

If the pressure of a mixture of 56 g of N_(2) and 44.0 g CO_(2) is 3 atm , the partial pressure of N_(2) in the mixture is :

Partial pressure of a vessel containing Cl_2 , CO_2 and CO is the sum of the partial pressure of Cl_2 , O_2 and CO . a) If so, is it correct to say partial pressure of a vessel containing NH_3 and HCl gases is the sum of their partial pressures? Justify

Calculate the total pressure in bar in a mixture of 8g of O_2 and 4g of H_2 confined in a vessel of 1dm^3 at 27^@C .

In Haber-Bosch process ammonia is manufacture by reacting H_2 and N_2 at 700 K and 200 atmosphere pressure. N_(2(g)) + 3H_(2(g)) harr 2NH_(3(g)) , DeltaH = -92 kJ The partial pressure of N_2 , H_2 and NH_3 are 2.09, 6.55 and 1.37 atm respectively. Calculate the value of K_P . And also explain the effect of increasing temperature on the value of K_P .

Thé total pressure of a mixture of O_2 and CO_2^ , in a container is given by the formúla, P_(Total)=P_(O_2)+P_(C O_2) a. Which law is used here? State the law. b. Can the total pressure of a mixture of 'NH_3(g) and HCl(g) taken in a container be determined using the formula. P_(Total) =P_NH_3+P_HCl . Why?

The total vapour pressure of a 4 mole % solution of NH_(3) in water at 293k is 50.0 torr, the vapour pressure of pure water is 17.0 torr at this temperature. Applying Henry's and Raoult's laws, calculate the total vapour pressure for a 5 mole% solution