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6. A power plant emits SO2 at a concentration of 1.00 g/mas S. In the atmosphere,...
6. A power plant emits SO2 at a concentration of 1.00 g/m3 as S. In the...
6. A power plant emits SO2 at a concentration of 1.00 g/m3 as S. In the atmosphere, SO2 reacts with water vapors to form H2SO3 and H;SO4. Assuming that a 40.0% of the emitted SO2 reacts to form H2SO3 and the rest of it reacts to form H2SO. a. Calculate the concentration of H2SO3 and of H2SO4. Express your answer in mol/m3 and g/m3 as S. b. Calculate the sum of the concentrations of H2SO; and H2SO4 Express your answer...
2. A power plant emits 300 kg of SO2 per hour into a neutral atmosphere with...
2. A power plant emits 300 kg of SO2 per hour into a neutral atmosphere with a wind speed of 2 m/s. The ơy and o, values are assumed to be 100m and 30m, respectively. Taken into consideration of the ground reflection effects: 1). what will the ground level concentration of SO2, expressed in ug/m3, if the town is 2 km off the plume centerline and the plant has a stack that produces an effective stack height of 20 meter?...
2. A power plant emits 300 kg of SO2 per hour into a neutral atmosphere with a wind speed of 2 m/s. The ơy and o, value...
2. A power plant emits 300 kg of SO2 per hour into a neutral atmosphere with a wind speed of 2 m/s. The ơy and o, values are assumed to be 100m and 30m, respectively. Taken into consideration of the ground reflection effects: 1). what will the ground level concentration of SO2, expressed in ug/m3, if the town is 2 km off the plume centerline and the plant has a stack that produces an effective stack height of 20 meter?...
A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour....
A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour. Most of the coal burned in the United States contains 1 to 4 % by weight sulfur in the form of pyrite, which is oxidized as the coal burns: 4FeS2(s) + 11 O2(g) 2 Fe2O3(s) + 8 SO2(g) Once in the atmosphere, the SO2 is oxidized to SO3, which then reacts with water in the atmosphere to form sulfuric acid: SO3(g) + H2O(l) H2SO4(aq)...
A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour....
A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour. Most of the coal burned in the United States contains 1 to 4 % by weight sulfur in the form of pyrite, which is oxidized as the coal burns: 4FeS2(s) + 11 O2 (g)--------> (Fe2O3(s) + 8 SO2(g) Once in the atmosphere, the SO2 is oxidized to SO3, which then reacts with water in the atmosphere to form sulfuric acid: SO3(g) + H2O(l) ----------> H2SO4(aq)...
Scientists determine the quantity of atmospheric sulfur dioxide (SO2), a large contributor to acid rain, by...
Scientists determine the quantity of atmospheric sulfur dioxide (SO2), a large contributor to acid rain, by an indirect titration. First, a scientist collects a sample of air and reacts it with hydrogen peroxide (H,O,) to form a solution of sulfuric acid ( H, SO2). Then, the amount of H, SO, produced is determined by titration with a sodium hydroxide solution (NaOH) of known concentration. H,02(aq) + SO2(g) → H, 50,(aq) H, SO (aq) + 2NaOH(aq) + 2 H2O(l) + Na,...
IReview I Constants Periodic Table The presence of SO2 in the atmosphere and the sulfuric acid...
IReview I Constants Periodic Table The presence of SO2 in the atmosphere and the sulfuric acid that it produces result in the phenomenon of acid rain. Uncontaminated rainwater is naturally acidic and generally has a pH value of about 5.6. The pH of acid rain is about 4 Part A This acidity has affected many lakes in northern Europe, the northern United States, and Canada, reducing fish populations and affecting other parts of the ecological network within the lakes and...
heet Pplete the following stoichiometry problems. Show ALL of your work to receive full credit. IOns and mole-to-mol...
heet Pplete the following stoichiometry problems. Show ALL of your work to receive full credit. IOns and mole-to-mole relationships 4Cr(s)+302(g)2Cr Os(s) How many moles of oxygen (02) would react with 0.35 moles of chromium (Cr)? a. b. Starting with 10.4g of O2, how many moles of Cr Os can be produced: How many grams of Cr metal would be needed to produce 38.2g of chromium (III) oxide? c. Sulfuric acid (H2SO4) is a component of acid rain which forms when...
Question 23 23. Consider the following chemical reaction: Zn(s) + 2H2SO4(aq) -> ZnSO4(aq) + SO2(g) +...
Question 23 23. Consider the following chemical reaction: Zn(s) + 2H2SO4(aq) -> ZnSO4(aq) + SO2(g) + 2H2O(1) 10.2 g zinc reacts with 45.0 ml. of sulfuric acid solution. Calculate molarity of sulfuric acid solution molar mass of Zn - 65.35 g/mole 6.94M 10.0M 3.00 M 0.422M 22. A sodium chloride solution is 15.0% m/m%. Calculate mass of sodium chloride in 219 g solution. 14.2g 80.3 g 32.98 11.2g
Consider the following reaction: 2H2S(g)+SO2(g)⇌3S(s)+2H2O(g) A reaction mixture initially containing 0.480 M H2S and 0.480 M...
Consider the following reaction: 2H2S(g)+SO2(g)⇌3S(s)+2H2O(g) A reaction mixture initially containing 0.480 M H2S and 0.480 M SO2 was found to contain 1.0×10−3 M H2O at a certain temperature. A second reaction mixture at the same temperature initially contains [H2S]= 0.255 M and [SO2]= 0.325 M . Calculate the equilibrium concentration of H2O in the second mixture at this temperature. Express your answer using two significant figures.
6. A power plant emits SO2 at a concentration of 1.00 g/m3 as S. In the atmosphere, SO2 reacts with water vapors to form H2SO3 and H;SO4. Assuming that a 40.0% of the emitted SO2 reacts to form H2SO3 and the rest of it reacts to form H2SO. a. Calculate the concentration of H2SO3 and of H2SO4. Express your answer in mol/m3 and g/m3 as S. b. Calculate the sum of the concentrations of H2SO; and H2SO4 Express your answer...
2. A power plant emits 300 kg of SO2 per hour into a neutral atmosphere with a wind speed of 2 m/s. The ơy and o, values are assumed to be 100m and 30m, respectively. Taken into consideration of the ground reflection effects: 1). what will the ground level concentration of SO2, expressed in ug/m3, if the town is 2 km off the plume centerline and the plant has a stack that produces an effective stack height of 20 meter?...
2. A power plant emits 300 kg of SO2 per hour into a neutral atmosphere with a wind speed of 2 m/s. The ơy and o, values are assumed to be 100m and 30m, respectively. Taken into consideration of the ground reflection effects: 1). what will the ground level concentration of SO2, expressed in ug/m3, if the town is 2 km off the plume centerline and the plant has a stack that produces an effective stack height of 20 meter?...
Scientists determine the quantity of atmospheric sulfur dioxide (SO2), a large contributor to acid rain, by an indirect titration. First, a scientist collects a sample of air and reacts it with hydrogen peroxide (H,O,) to form a solution of sulfuric acid ( H, SO2). Then, the amount of H, SO, produced is determined by titration with a sodium hydroxide solution (NaOH) of known concentration. H,02(aq) + SO2(g) → H, 50,(aq) H, SO (aq) + 2NaOH(aq) + 2 H2O(l) + Na,...
IReview I Constants Periodic Table The presence of SO2 in the atmosphere and the sulfuric acid that it produces result in the phenomenon of acid rain. Uncontaminated rainwater is naturally acidic and generally has a pH value of about 5.6. The pH of acid rain is about 4 Part A This acidity has affected many lakes in northern Europe, the northern United States, and Canada, reducing fish populations and affecting other parts of the ecological network within the lakes and...
heet Pplete the following stoichiometry problems. Show ALL of your work to receive full credit. IOns and mole-to-mole relationships 4Cr(s)+302(g)2Cr Os(s) How many moles of oxygen (02) would react with 0.35 moles of chromium (Cr)? a. b. Starting with 10.4g of O2, how many moles of Cr Os can be produced: How many grams of Cr metal would be needed to produce 38.2g of chromium (III) oxide? c. Sulfuric acid (H2SO4) is a component of acid rain which forms when...
Question 23 23. Consider the following chemical reaction: Zn(s) + 2H2SO4(aq) -> ZnSO4(aq) + SO2(g) + 2H2O(1) 10.2 g zinc reacts with 45.0 ml. of sulfuric acid solution. Calculate molarity of sulfuric acid solution molar mass of Zn - 65.35 g/mole 6.94M 10.0M 3.00 M 0.422M 22. A sodium chloride solution is 15.0% m/m%. Calculate mass of sodium chloride in 219 g solution. 14.2g 80.3 g 32.98 11.2g
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