QUESTION 4 A flask has 1.50 moles of hydrogen gas at 30.0 °C and a pressure of 375 mm Hg. After the addition of more hydrogen gas at the
same temperature, the pressure rises to 1.50 atm. How many moles of hydrogen gas are added? 1 atm - 760 mm Hg.

Be sure to answer all parts. the following equilibrium constants were determined at 1123 k: c(s) + co2(g) ⇌ 2co(g) k'p = 1.30 × 1014 co(g) + cl2(g) ⇌ cocl2(g) k''p = 6.00 × 10−3 calculate the equilibrium constant at 1123 k for the reaction: c(s) + co2(g) + 2cl2(g) ⇌ 2cocl2(g) 4.68 × 10 9 (enter your answer in scientific notation.) write the equilibrium constant expression, kp: