Calculate "delta" S for the following reaction: H2(g) + Br2(l) --> 2HBr(g) given: S[H2(g)] = 0.131 kJ/K S[Br2(l)] = 0.152 kJ/K S[HBr(g)] = 0.199kJ/K a. 0.482 kJ/K b. 0.681 kJ/K c. 0.115 kJ/K d. -0.084 kJ/K e. 0.084 kJ/K
For the second order reaction below, the concentration of A after 125 seconds is 0.0722M. If k=9.11x10(exponent negative 2) seconds(exponent negative 1), what ws the initial concentration of A? 2A-->B
Finding molarity and answering questions on the reactions and productions of a balanced equation
1.) What is the molarity of a solution made by dissolving 25.6 g of KOH (5601 g/mol) in enough water to make 3.00 L of solution? 2.) 2 Fe + 3 Cl2 ------> 2FeCl3 How many moles of Fe are needed to produce 76.4 g of FeCl3 (162.3 g/mol)? How many grams of Fe (55.8 g/mol) are needed to react with 123 g or cl2 (71.0 g/ ...continues
Rate of radioactive decay-half life
How many atoms decay in 24 hours in a 2.5 x 10(exponent negative 6) Ci source? 1 Ci=3.700 x 10(exponent 10) atom/s. Please show how you arrive at the solution. thanks a. 0.22 atoms b. 1.3 x 10(exponent 21) atoms c. 9.3 x 10(exponent 4) atoms d. 2.3 x 10(exponent 6) atoms e. 8.0 x 10(exponent 9) atoms
A 1.00g of sample of Ge decays to 0.87 in 1.9hr. What is the half-life of Ge? Please show how you arrive at the solution. thanks a. 1.4 x 10(exponent 1)hr b. 9.5 hr c. 1.1 x 10(exponent negative 1) hr d. 7.3 x 10(exponent negative 2) hr e. 13 hr
The half life of Cl is 9.5 x 10(exponent 12)s. How many atoms of Cl are present in a sample with an activity of 1.5 x 10(exponent 9) atoms/s a. 2.1 x 10(exponent 22) atoms b. 6.3 x 10(exponent 3) atoms c. 4.9 x 10(exponent negative 23) atoms d. 1.4 x 10(exponent 22) atoms e. 7.0 x 10(exponent 23) atoms
Pu decays by alpha emission. The isotope's half-life is 2.4 x 10(exponent 4) yr. How many alpha particles are emitted per second by 25mg of Pu?
In spontaneous nuclear reactions: a. the products weigh less than the reactants b. the products weigh more than the reactants c. the difference in mass between reactants and products is zero d. mass is converted to light e. the products move at the speed of light squared
A 1.000g sample of an unknown hydrocarbon containing only carbon and hydrogen is burned in excess oxygen to yield carbon dioxide and water. The masses of CO2 and H2O are 2.994g and 1.635g, respectively. What is the empirical(simplest) formula for this compound?
1.) How many bonds are present in propene, C3H6? 2.) How many bonds are present in acetylene, C2H2?
