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Suppose that 0.35 mol of hydrogen gas and 0.35 mol of clorine gas are placed in a 1L reaction vessel at a certain temperature, and the following reaction comes to equilibrium:
H2(g) + Cl2(g) revrxnarrow.gif 2HCl(g)
How many moles of hyrdogen chloride are there in the reaction vessel at equilibrium?
A 1-L flask is filled with 1.30 g of argon at 25 degrees Celsius. A sample of ethane vapor is added to the same flask until the total pressure is 1.05 atm. What is the partial pressure of argon in the flask?
Determine the Osmotic Pressure for the following aqueous solutions @ 25 degrees Celsius. (a.) 1.0. M Glucose, and (b.)1.0 M NaCl. Explain which solution has the greater osmotic pressure if any and why.
63.0 mL of a 1.20 M solution is diluted to a volume of 208 mL. A 104-mL portion of that solution is diluted using 157 mL of water. What is the final concentration.
1. How many CO2 molecules are needed to produce 1 glucose molecule (in photosynthesis)? 2. How many moles of oxygen atoms are in 1 mole of calcium phosphate?
What is the purpose of running both Dalton Vll mixed markers and lanes with individual markers on SDS-PAGE?
Finding Number of Atoms in a Molecule from Molecular Weight, As determined from the gas law, the molecular weight of a substance is eight times the atomic weight
Compute the molecular formula of CH 3 COOH the percent composition of acetic acid is 39.99% C and 6.73% H. The remainder of the compound is oxygen.(The molar mass of acetic acid is 60.06 g/mol.)
Calculate the mole fraction of the salt in the solution.
how do you find the empirical formula of a compound if they don't give you percentages. For example, if they ask: what is the empirical formula for N2O4?
What mass of helium gas is needed to pressurize a 112.0 L tank to 262 atm at 25°C?
Calculating the equilibrium constant (Keq) for the given reactions - Determine the Keq for the following reactions
calculate the mass of silver chloride and dihydrogen monosulfide formed when 85.6 grams of silver sulfide reacts with excess hydrochloric acid.
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