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How much water would be needed to completely dissolve 1.65 L of the gas at a pressure of 745 torr and a temperature of 18 C?
determine the energy change that occurs during the combustion of 1 mole of ethene (ethene's connectivity is: H2C=CH2 also written as CH2=CH2).
Determine the mass of propylene glycol neded to substitute one gallon of ethylene glycol and also find out the volume of propylene glycol, required to get the same antifreeze protection as one gallon of ethylene glycol.
What is the product expected from the reaction of 1.3-butadiene and 3-sulfolene. Why is this not a major concern as a by product
Ammonia is made industrially by reacting nitrogen and hydrogen under pressure, at high temperature, and in the presence of a catalyst. The equation is N2(g)+3H2(g)---->2NH3(g). If 4.0mol of H2 react, how many moles of NH3 will be produced.
Consider the reaction with the rate law, Rate = k[BrO3-][Br-][H+]2 By what factor does the rate change if the concentration of Br- is doubled? Just put in the number as a whole number or fraction.
15.0mL of 0.50 HCl is added to a 100.0mL sample of 0.200 M HNO2. What is the equilibrium concentration of NO2. ions. (Ka for HNO2= 4.0 x 10^-4)
How many moles of H3O+ must be added to one liter of a solution to adjust the pH from 7.48 to 5.90?
The system H2 (g) + I2 (g) ?? 2 HI(g) is at equilibrium at a ?xed temperature with a partial pressure of H2 of 0.200 atm, a partial pressure of I2 of 0.200 atm, and a partial pressure of HI of 0.100 atm.
At a Concentration of 1M, the weak acid HN0 is 2% ionized and the pH of the solution is 1.7 . What happens when KNO2(s) is dissolved into the solution: The extent of HNO2 ionization = Increases or decreases? The concentration of H+ = Increases or ..
the world's estimated annual gas reserves in 2006 were 6124 trillion ft3 .The world rate of annual use was 105.5 trillion feet3. How long these reserves will last if the rate of use continues?
2121g sample of an organic compound was burned in a stream of oxygen adn the CO2 produced was collected in a solution of barium hydroxide. Calculate the percentage of carbon in the sample if .6006 g of BaCO3 was formed
determined the limiting reactant and the theoretical yield (in g) of nitrogen that can be formed from 24.0 g N2O4 and 23.5 g N2H4 molar masses are as follows: n2o4 92.02 n2h4 32.05
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