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- What mass of phosphorus is present in 25 g P4S3?A. 14gB. 4.5gC. 11gD. 3.2gE. 100gIn the reaction X + 3 Y → 2 Z, the mass of X is 5.0 g and the mass of Z is 14.0 g. If the reaction was carried out again and the mass of Z produced was 7.0 g, what mass of Y reacted? a. 7.0 g O b. 2.5 g C. 9.0 g d. 4.5 gA 23.4 g23.4 g sample of magnesium reacts with excess silver nitrate to produce silver metal and magnesium nitrate. The reaction is stopped before all of the magnesium metal has reacted. A total of 62.6 g62.6 g of solid metal is present. Calculate the mass of each metal in the 62.6 g62.6 g mixture.
- What volume of 3.51 M KOH is required to prepare 211.0 mL of 0.750 M KOH?a. 1.24 × 10–2 mLb. 5.55 × 102 mLc. 80.2 mLd. 45.1 mLe. 9.87 mLCalculate the mass of Na in 80.0 g NaCl.A. 31.5 gB. 6.2 gC. 40.0 gD. 1.9 gThe required volume of 28.0 (w/w) % ammonium hydroxide (density =0.899g/mL) diluted it up to 500.0 mL to make 0.250 M NH3 (NH3 RMM=17.03 g/mol) is a. 7.62 mL b. 23.67 mL c. 8.46 mL d. 10.56 mL
- Butane (C4H10) plus Oxygen yields carbon dioxide plus water. b. Balance the chemical equation. 2C4H10(g) + 13O2(g)→ 8CO2(g) + 10 H2O(g) c. What type of chemical reaction is it? d. Is this a physical or a chemical reaction? Please justify your answer by providing evidence from the chemical equation.The formula for carbon monoxide is CO. a. How many molecules are in 3.35 grams of carbon monoxide? molecules b. What is the mass in grams of 3.58 x 1022 molecules of carbon monoxide? gramsa. A 250.0-mL solution of sodium hydroxide was prepared by dissolving pure NaOH(s) in deionized water. It required 21.37 mL of 0.1127 M sulfuric acid to completely neutralize 39.29 mL of this sodium hydroxide solution. Calculate the mass, in units of g, of NaOH(s) that was dissolved to make the 250.0-mL solution. Enter your answer in decimal notation using 3 significant figures; i.e., enter 0.03478 as 0.0348 b. In an experiment, 23.24 mL of 0.235 mM silver nitrate are mixed with 9.12 Ml of 0.205 mM sodium phosphate. Assuming 100% yield, what is the concentration, in units of μM, of phosphate in the solution. Assume that the volume of the solid formed is negligible. Enter your answer in decimal notation using 3 significant figures; i.e. enter 2.579 as 2.58.
- A college chemistry student is performing this reaction in a lab, where magnesium is burned and combines with oxygen from the air to produce magnesium oxide. The students burns 2.92 g of Mg, and there is excess oxygen from the air. They incorrectly 'culated that the mass of magnesium oxide produced was 2.42 g. Here is their work: 2.92 g 1 mol 2 mol 40.3 g = 2.42 g 1 24.3 g 1 mol 1 mol 1) What did the student do wrong? There is an error in their work. Explain specifically what part is incorrect. 2) What recommendation(s) would you give to the student regarding showing their work? There is an improvement that can be made to help them avoid this mistake in the future. pts) 3) Instead of 2.42 g, what answer should the student have gotten?5. The density of water at 4.00°C is 0.967 g/mL. How many molecules of water are present in a 499.8 mL bottle of water? Express your answer to the correct number of significant figures. Be sure to show all steps completed to arrive at the answer. 1.615 X 105 molecules water, to solve the equation you can calculate the mass and the water and then convert It to moles and then you calculate the number of moleculesIn the standardization of NaOH solution, 0.5211 g potassium hydrogen phthalate (204.22 g/mol) is used to neutralize 23.65 mL of NaOH solution. Calculate the molarity of the NaOH solution. OA. 0.1079 M O B. 0.1231 M O.0.07815 M O D.7.8 x 10-5 M ОЕ 1.1 х 104 м