When nitrogen dioxide from car exhaust combines with water in the atmosphere, it forms nitric acid and nitrogen monoxide. 1) Balance the equation __NO2+ __H2O --> __HNO3 + __NO 2) When 4.50 kg of nitrogen dioxide reacts with an excess of water, how many grams of nitric acid can form?

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What is the mass of the initial sample burned?

Balance the following chemical equation. Note that a empty blank space will be interpreted as "1."   ___N2H4 (g) + ___N2O4 (g)  -->  ___N2 (g)  + ___H2O (g)

80.0 grams of I2O5 (molar mass 333.80g/mol), reacts with 38.0 grams of carbon monoxide (molar mass 28.01g/mol). Determine the mass of iodine that could be produced.  balanced equation I2O5+5CO ----> 5CO2+I2

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo

Balance the following equation.   ___N2H4(g) + ___H2O2(g) → ___N2(g) + ___H2O(g)

Al2O3 + 2Fe -------> Fe2O3 + 2Al   How many moles of Iron (III) oxide is produced from if 8.2 moles of Iron is used to react with aluminium oxide.

Question 25 of 97 Submit DDT was an insecticide used to prevent mosquito borne diseases. Due to the harmful effects on birds and fish, it is now banned in the US. However, other countries still use it to control mosquitos. It can be prepared by the reaction shown below. Determine the amount of DDT that can be produced and the percent yield for this reaction. 2C6H,CI + C2HOCI, – C,4H9CI, + H20 2 3 NEXT If a company in South America started with 1175 g of chlorobenzene (C6H5CI, MW 112.55 g/mol) and 538.5 g of chloral (C2HOCI3, MW 147.39 g/mol), set up the table below that represents 100% yield with the given reaction conditions. 2C6H,CI C2HOCI, C1.H,Cls H2O Before (mol) Change (mol) After (mol) O RESET 3.132 -3.132 3.654 -3.654 7.308 0. + -7.308 10.44 -10.44 MacBook Air F12 II F8 F10 F11 000 F9 20 F3 F7 F4 F5 F6 esc F2 F1 +.

Use balanced chemical equations to relate amounts of reactants and products. The unbalanced equation for the reaction between perchloric acid (HCIO4) and tetraphosphorus decaoxide is shown below. Balance the equation (enter the smallest integer possible in each box, including the integer "1" when needed) and determine the amount of P4010 consumed and the amounts of H3PO4 and Cl₂07 produced when 0.805 mol of HCIO4 reacts. HCIO4 (aq) + P4010 (S) mol P4010 consumed mol H3PO4 produced mol Cl₂O7 produced H3PO4 (aq) + Cl₂07 (1)