If you don't reply with an actual answer i will report it and you will be reported and itll give me back my points 1.if i have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature? 2.if i have an unknown quantity of gas at a pressure of 121.6 kpa, a volume of 31 liters, and a temperature of 87 0c, how many moles of gas do i have? 3.if i contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 k, what is the pressure inside the container? 4.if i have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0c, what is the volume of the container that the gas is in? 5.if i have 17 moles of gas at a temperature of 67 0c, and a volume of 88.89 liters, what is the pressure of the gas? use dalton’s law of partial pressures and grahams law of effusion to solve the following problems: 6.at a certain temperature, molecules of methane gas, ch4 have an average velocity of 0.098 m/s. what is the average velocity of carbon dioxide molecules at this same temperature? 7.7.) find the relative rate of diffusion for the gases chlorine, cl2 and ethane, c2h6. 8.495 cm3 of oxygen gas and 877 cm3 of nitrogen gas, both at 25.0 °c and 114.7 kpa, are injected into an evacuated 536 cm3 flask. find the total pressure in the flask, assuming the temperature remains constant.

Answeropposite;

Answer is: the equilibrium  shifts toward the reactants, to the left side of chemical reaction.it is because lead(ii) nitrate dissociates in water: pb(no₃)₂ → pb²⁺(aq) + 2no₃⁻(aq).according to lechatelier's principle, the position of equilibrium moves to counteract thechange (more lead cations, common ion), the position of equilibrium will move so that the concentration ofproducts decrease and concentration of reactants of chemical reaction increase.read more on -

Answerchemical energy;

Note that 2 mol dm⁻³ = 2 mol/(dm³)outline: we're given the concentration of hcl, which is  2 mol dm⁻³ (cubic meters in the denominator can represent volume, so i know this is concentration). we're an amount of calcium carbonate caco₃, which is 5 g. we're presented with a chemical equation which includes caco₃ and hcl. we are told to find the volume of hcl. from what we see so far, this seems to be a stoichiometry  problem. we'll have to use the given information about calcium carbonate to find the amount of moles of hcl needed to fully react with calcium carbonate. then we'll have information about the moles of hcl and the concentration of hcl; that will be enough to figure out volume according to the formula concentration = moles / volume.======all the answer choices are not in dm.convert the given concentration so that it uses cm⁻³.we can use conversion factors. we have to cube our conversion factors so that dimensional analysis works.we can convert to meters first, using the fact that     10 dm = 1 m  ⇔ 10³ dm³ = 1 m³then we use the fact that     10² cm = 1 m ⇔ (10² cm)³ = (1 m)³ ⇔ 10⁶ cm³ = 1 m³so converting:     now we have to find the moles of hydrochloric  acid neededfind the moles of calcium carbonate. we have to find the molar mass of calcium carbonate, caco₃, which can be found by    molar mass = (mass ca) + (mass c) + 3(mass o)    = 40 + 12 + 3(16)    = 100 g/molconvert the given 5 g to moles:     mol caco₃ = 5 g caco₃ * 1 mol/(100 g) = 0.05 mol caco₃use stoichiometry (ratios) to figure out the moles of hcl needed. ratio wise, there's 2 hcls for every caco₃, so use dimensional analysis    mol hcl = mol caco₃ * (2 mol hcl) / (1 mol caco₃)    = 0.05 mol hcl * 2    = 0.1 mol hcl  we have 0.1 mol hcl and concentration of hcl (0.002 mol/cm³).we need to find volumesince concentration = moles / volume, rearrange to get     volume = moles / concentration    volume = 0.1 mol / (0.002 mol/cm³)    volume = 50 cm³