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When moles of a s grams is dissolved in grams of water at c the temperature of the


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1.Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called " NOx ") that are of interest ...

of interest to atmospheric chemistry. It can react with itself to form another form of NOx , dinitrogen tetroxide. A chemical engineer studying this reaction fills a 125L tank with 40.mol of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 18.mol of nitrogen dioxide gas. The engineer then adds another 10.mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.
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2.3A(g) + X(g) → Z(g) ΔH° = -480 kJ/molrxn The equation shown above represents an exothermic reaction between A(g) ...

reaction between A(g) and X(g). What is the amount of heat released when 10 mol of A(g) reacts with an excess X(g) ? ΔH A -236kJ X -136kJ Y -167kJ Using the heats of formation found in the table above, calculate ΔH for the reaction below. 6A(aq) + 7X(g) → 6Y(l) Y + 2X → 4Z ΔH=-4 A + 3B → 2Z ΔH=-2 A → X +C ΔH=7 Using the thermodynamic data above, determine ΔH for the reaction below. 2C+ 6B → Y When 0.3 moles of A(s) (4 grams) is dissolved in 12 grams of water at 23°C, the temperature of the water increases to 31°C. The specific heat of water is 4.18 J/g°C. Calculate ΔH in kJ/mol. Report your answer to 1 decimal place.
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3.1) A hypothetical element exists as two isotopes: I = 42.00 amu and II = 49.00 amu. If the percent ...

bundance of isotope I is (1.94x10^1)%, what would be the calculated atomic mass (in amu)? 2) A hypothetical element exists as two isotopes: I = 78.00 amu and II = 84.00 amu. If the atomic mass of this element is found to be 80.33 amu, which isotope must be more abundant? 3) If the hypothetical polyatomic ion ThOM2- is called "thomite", what would be the formula and name of the acid formed by this ion? 4) How many atoms of hydrogen are there in a sample of (4.00x10^2) grams of NH3(g)? 5) How many O (oxygen) atoms are there in (6.40x10^2) grams of H3PO4? 6) How many moles of fluorine atoms are there in (5.80x10^2) grams of SF4? 7) When 3.50 g of titanium (Ti) reacts with oxygen, the resulting oxide compound weighs 5.84 g. What is the empirical formula of this oxide? 8) How many moles of molecules are there in (6.70x10^2) grams of CH4? 9) A chemical is found to be 80.0% C and the rest is H. If the molar mass of this chemical is known to be 90.2 g/mol, what is the molecular formula?
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1.AU MAT 120 Systems of Linear Equations and Inequalities Discussion

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