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Using a sample having 1.50mL of nitroglycerin(NG) that has density=1.592g/mL then calculate how many total moles of gas are produced?
Ethyl mercaptan C2H6S(The volatile liquid) is knows as one of the most odoriferous substances and It may be combined with natural gas to make leaks detectable. Calculate how many molecules of C2H6S (ethyl mercaptan )are contained in 1.0 micro liter sample if the given density = 0.84 g/mL
Compute the pH if NaOH solution of the 10.00 mL has been mixed. pKa of HCOOH = 3.74
In which compound does sulfur have the highest oxidation number a)Na2S2O3 b)NaHS c)H2S d)KHSO3 e) CuSO4
Calculate how many moles of nitrogen will be required to make 10.0 moles of NH 3 and calculate what is energy of each pulse If each pulse contains no of photons =1.20 x 10 18
Compute the free energy change needed for transport of sufficient protons to make gastric juice of 1 litter at the temperature of 37 degree celsius hence expect above reaction will happen spontaneously?
Determine how many moles of carbon dioxide should be added to the system to bring the equilibrium carbon monoxide concentration to 0.743 mol/L
Write the structure of the conjugate acid of this base while consider the base monosodium phosphate, Na (HO)2P( O)O also explain why an aqueous solution of monosodium phosphate would be ineffective for extracting benzoic acid? pKa of this conjugat..
Assuming all gases are at the same pressure and temperature, how many liters of CO2 are formed from 15.0L of CO.
Calculate what the limiting reactant is in the reaction between copper (II) oxide and hydrochloric acid
Calculate the rate constant for the reaction when the reactant concentration in a first-order reaction is given 7.30×10-2M after 15.0s and it is also reported 4.40×10-3M after 65.0s . ?
Questions on chemical equations - Write a balanced equation for this reaction. Include the states of matter for each compound.
Multiple choice questions in Radioactive Decay - electron emitted from the nucleus during some kinds of radioactive decay is known
A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Compute the pH of the solution before the addition of any HNO3. Kb of NH3 =1.8 × 10-5.
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