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1 - A calorimeter has a heat capacity of 3.35J/C. Calculate the quantity of heat required to raise the temperature of this calorimeter from 4c to 175c.
2 - 4500J of heat are absorbed by a calorimeter. The temperature of the calorimeter increases from 14c to 121c. Calculate the heat capacity of the calorimeter.
Write a balanced equation and an expression for Ksp for the dissolution of the given ionic compound. Include states-of-matter. CaCO3 balanced equation: solubility expression
Your intuition probably tells you that for 2 identical blocks, Tf is the average of the initial temperatures, so that Tf = 1/2 (T1 + T2)
Compute delta Hf for CaC2 : CaC2 + 2H2O-->Ca(OH)2 +C2H2 From the given enthalpy of reaction data as water(H2O) =(2*-285.83),calcium hydroxide Ca(OH)2=(-986.2) , AcetyleneC2H2 =(226.77)?
Concentrated sulfuric acid is 98% by mass H2SO4, with the remaining mass being water. What is the molar concentration (i.e., molarity) and the molal concentration (i.e., molality)
What is the ratio of HCO3- to H2CO3 in an exhausted marathon runner whose blood pH is 7.1? Note: There is no need to consider the Ka2, use only the Ka1.
A solution is made by mixing equal masses of methanol, CH4O, and ethanol, C2H6O. Determine the mole fraction of each component to at least three significant figures.
It required 50.00 mL of 0.1565 M KMnO4 to titrate 2.878 g of the solution containing hydrogen peroxide. What was the mass percentage of H2O2 in the solution
An experiment requires 42.5 g of sulfuric acid, which is easier to measure by volume than by mass. What volume in mL should be measured out, if the density of the sulfuric acid is 1.84 g/cm^3
When a 58.4 nm radiation is directed on a sample of Krypton, electrons are ejected with a velocity of 1.59x106 m/s. What is the ionization energy of the Krypton
using a sample of 21.004 grams of aqueous waste leaving a fertilizer manufacturer has nh3 ammonia. is diluted with h2o
Write net Brønsted equations that show the acidic or basic nature of the following substances, given the pH.
When adding the solution of HNO3 from the buret in Step 14 to beaker 4, you know that you added 2.5 mL instead of 1.5 mL for a total volume of 11.0 mL. How would the calculated value of the equilibrium constant be affected for this sample?
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