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Octane has a specific heat of 2.22 J/g.K. (a) How many joules of heat are needed to raise the temperature of 40.0 g of octane from 10.0 oC to 40.0 oC? (b) Which will require more heat, increasing the temperature of 1 mol of octane by 10 degrees or increasing the temperature of 1 mol of water by 10 degrees
Sulfur dioxide reacts with chlorine at 227 oC: SO2(g) +Cl2(g) ↔ SO2Cl2(g) Kp for this reaction is 5.1 x 10-2 atm-1. Initially, 1.00 g each of SO2 and Cl2 are placed in a 1.00 L reaction vessel.
Calculate the radiation dosage (in grays) for an 57-kg person that is exposed for 3.0 seconds to a 3.0 Ci source of beta radiation.
A Solution is made by dissolving 8.5 grams of NaOH in 2.3 L of water. What is the molarity of the solution?
The catalytic converter on your automobile contains small amounts of a precious metal catalyst. Which of the following components would you expect to be decreased in your tailpipe emissions.
Calculate the density of N2 at STP, (a) using the ideal-gas law and (b) using the molar volume and molar mass of N2.
draw an orbital picture for acetylene C2H2 label each bond type and indicate type of orbitals involved in each bond.
A steel cylinder holds 150.0 mol argon gas at 25 degrees C and a pressure of 9.53Mpa. After some argon has been used, the pressure is 2.00Mpa at 19 degrees C. What mass of argon remains in the cylinder.
Calculate the degree of unsaturation number of missing H2 units relative to an alkane for the Compound with the molecular formula C 16 H13 N2 O CI Enter your response as an integer number
Given that K for the following reaction equals 2.2. Calculate K for the reverse reaction. SO2(g)+1/2O2(g) SO3(g). Please explain the steps so I can understand.
0.3 M NaH2PO4 calculate acidic and basic buffer capacity. How muc of strong base needed to bring buffer pH one unit up?
how to draw the Lewis Structure for this. The complete questions says: "Lithium aluminum hydride, LiAlH4, contains both ionic
Halogenated compounds are particularly easy to identify by their mass spectra because chlorine and bromine occur naturally as mixtures of two abundant isotopes
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