Only need help with subpart "d" Use the following data and steps below to calculate the formula of the copper chloride hydrate. Empty aluminum pan was 0.4661 g. A 0.8390 g sample of CuCl2*xH20 was placed in the pan and heated. The final mass of the brown CuCl2 in the aluminum pan was 1.1357 g. a. How many moles of water evaporated? 0.00941 b. Calculate the moles of dry copper chloride. 0.00498 c. How many water per copper chloride? Round it to the nearest whole number and determine the formula of the starting hydrate. 2 d. A common hydrate for copper (II) chloride is the di-hydrate: CuCl2×2(H2O). Assume that the starting hydrate was this and calculate the theoretical yield of anhydrous copper chloride.
Only need help with subpart "d"
Use the following data and steps below to calculate the formula of the copper chloride hydrate. Empty aluminum pan was 0.4661 g. A 0.8390 g sample of CuCl2*xH20 was placed in the pan and heated. The final mass of the brown CuCl2 in the aluminum pan was 1.1357 g.
a. How many moles of water evaporated? 0.00941
b. Calculate the moles of dry copper chloride. 0.00498
c. How many water per copper chloride? Round it to the nearest whole number and determine the formula of the starting hydrate. 2
d. A common hydrate for copper (II) chloride is the di-hydrate: CuCl2×2(H2O). Assume that the starting hydrate was this and calculate the theoretical yield of anhydrous copper chloride.
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