When 109.27 g of pure copper reacts with 488.28g of iodine, 546.35g of a compound containing only copper and iodine result. 51.20g of iodine remain when the reaction is complete.
a. Do these results support the Law of Conservation of Mass? Explain
b. Another student heat 5.10g of copper with 7.00g of iodine.The product is a white compound with mass of 10.50g with 1.60g of copper left over. Is the compound made in this experiment, the same or different than the first one? If different prove that these two experiments together support the Law of multiple proportions.
When 109.27 g of pure copper reacts with 488.28g of iodine, 546.35g of a compound containing...
In a lab experiment, 8.24 g of phosphorus reacts with bromine to form 72.01 g of phosphorus tribromide. (a) Calculate the percentage by mass of P in phosphorus tribromide. (b) How many grams of bromine reacted? How do you know? law of definite proportions law of multiple proportions law of constant composition law of conservation of mass
In a lab experiment, 6.3 g of Mg reacts with sulfur to form 14.6 g of magnesium sulfide. (a) Use the equation below to calculate the percentage by mass of Mg in magnesium sulfide. % X component amount of component x 400 total amount (b) How many grams of sulfur reacted? How do you know? law of constant composition law of conservation of mass law of definite proportions law of multiple proportions Need Help?
In a lab experiment, 6.9 g of Mg reacts with sulfur to form 16.0 g of magnesium sulfide. (a) Use the equation below to calculate the percentage by mass of Mg in magnesium sulfide. % X component = amount of component x.. total amount 4.9 % (b) How many grams of sulfur reacted? 49 How do you know? O law of constant composition O law of definite proportions O law of multiple proportions O law of conservation of mass
multiple proportions. Explain your reasoning. 4. Magnesium reacts with oxygen to produce magnesium oxide, a white powder. A) In one experiment, 2.50g of magnesium reacts with 1.38g of oxygen to form 3.48g| magnesium oxide; all of the oxygen is consumed, but some magnesium is left over. Calculate (1) the mass of magnesium in the magnesium oxide; (2) the Mg/O ratio. B) In another experiment, 2.85g of magnesium reacts with 4.00g of oxygen to form 4.73g of magnesium oxide; all of...
A compound containing sulfur and fluorine contains 8.00 g of S and 9.50 g of F. Which combination of S and F masses represents a different compound that obeys the Law of Multiple Proportions? Group of answer choices a. 4.00 g of S and 4.75 g of F b. 32.0 g of S and 38.0 g of F c. 8.00 g of S and 10.5 g of F d. 16.0 g of S and 57.0 g of F
Calculate the heat evolved when 0.500 g of Cl, (g) reacts with an excess of HBr (g) to form HCI (g) and Br, (0, given the following standard enthalpies of formation (kJ/mol): HCI (B), - 92.30; HBr (g), -36.20. Ryan Experiment 4 Advance Study Assignment: Determination of a Chemical Formula 1. To find the mass of a mole of an element, one looks up the atomic mass of the element in a table of atomic masses (see Appendix III or...
1. When 2.50 g of copper metal reacts with molecular oxygen, the copper oxide product of the reaction has a mass of 2.81 g. What is the empirical formula of the copper oxide product 2. When 10.8 g of silver was reacted with sulfur. 12.4 grams of product was produced there was only one product). What is the empirical formula of the product? 3. Lysine is a compound composed of carbon, hydrogen, nitrogen and oxygen. When 1.50 g of lysine is burned,...
When 1.3213 g of an organic iron compound containing Fe, C, H, and O was burned in O2, 2.4714 g of CO2 and 0.70728 g of H2O were produced. In a separate experiment to determine the mass percent of iron, 0.6161 g of the compound yielded 0.1392 g of Fe2O3. What is the empirical formula of the compound?
When 1.4083 g of an organic iron compound containing Fe, C, H, and O was burned in O2, 2.6341 g of CO2 and 0.75385 g of H2O were produced. In a separate experiment to determine the mass percent of iron, 0.4231 g of the compound yielded 0.09559 g of Fe2O3. What is the empirical formula of the compound?
When 1.1338 g of an organic iron compound containing Fe, C, H, and O was burned in 02, 2.1207 g of CO2 and 0.60692 g of H2O were produced. In a separate experiment to determine the mass percent of iron, 0.6461 g of the compound yielded 0.1460 g of Fe,O3. What is the empirical formula of the compound?