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How much energy is required to completely vaporize a gallon jug of ice (128g) at 0C in 10 seconds? (in kilojoules)
What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires
Metals such as magnesium and zinc react with dilute sulfuric acid to give hydrogen, according to the equation: M (s) + H2SO4 (aq) -------> MSO4 (aq)
The resulting solution is titrated to a starch endpoint with 34.81 mL of the thiosulfate solution. Calculate the concentration of the thiosulfate solution.
A block of metal has a width of 3.2 cm, a length of 17.1 cm, and a height of 2.7 cm. Its mass is 1.5 kg. Calculate the density of the metal. Express in grams per cubic centimeter using two significant figures.
How many liters of NO(g) can be made from 17.57 L of O2(g) and 16.55 L of N2(g) at STP?
Calcium carbide reacts with water to form acetylene and calcium hydroxide. From the following enthalpy data calculate Delta Hf for CaC2
calculate how many moles of KIO3 are needed to make 50 ml of 0.20 M solution?
An endothermic chemical reaction with ?E = +41 kJ/mol has an activation energy of +95 kJ/mol. What is the activation energy for the reverse reaction
In the unbalanced reaction, Sn + HNO3 ---> Sn(NO3)2 + H2), 2.100 grams of Sn(NO3)2 was formed. How many grams of NO were formed and how many moles of HNO3 were reacted? (HINT: the coefficient of Sn is 3).
The mass spectrum of an organic compound shows the relative abundances of M to be 62.87% and M 1 to be 4.760%. Assuming the peaks are caused by 12C and 13C isotopes,
If it were possible to obtain 100% yield, when the temperature was returned to the origenal value what would be the partial pressure of each gas be?
Estimate Delta G or this reaction at each of the following temperatures. (Assume that Delta H and Delta S do not change too much within the given temperature range.)
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