15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to
drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? Name the hydrate
Problem #1: A 15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? Solution: 1) Determine mass of water driven off: 15.67 minus 7.58 = 8.09 g of water 2) Determine moles of MgCO3 and water: MgCO3 --> 7.58 g / 84.313 g/mol = 0.0899 mol H2O --> 8.09 g / 18.015 g/mol = 0.449 mol 3) Find a whole number molar ratio: MgCO3 --> 0.0899 mol / 0.0899 mol = 1 H2O --> 0.449 mol / 0.0899 mol = 5 MgCO3 · 5H2O
15.67 g sample of a hydrate of magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate? Name the hydrate
Question five A 15.67 g sample of a hydrate of magnesium carbonate ( MOONH:O) was heated without decomposite the carbonate, to drive off the water. The mass was reduced to 7.58 g (Molar mass of MgCO: - 84313 Smol) (5 mark) A. What is the formula of the hydrate? B. Determine the percentate in the hydrated sit
An experiment was performed to determine the percentage water content in a hydrated compound. A 15.67 g sample of a hydrate, magnesium carbonate was heated, without decomposing the carbonate, to drive off the water. The mass was reduced to 7.58 g. What is the percent water content?
please help me solve all 3! Thank you in advance A 15.67 g of a hydrate of magnesium carbonate was carefully heated to drive off the waters of hydration. The mass was reduced to 7.58 g after the water was driven off. What is the molecular formula of this hydrate? Complete the molecular formula by choosing the appropriate coefficient below: MgCoz v H20 Checl OVO AWN Next page Silver nitrate has the molecular formula AgNO3. In a 216.8 g sample...
A 1.232 g sample of a magnesium sulfate hydrate is heated until its final mass is 0.602 g. What is the formula of the hydrate? Note: the molar mass of MgSO4 is 120.4 g/mol and the molar mass of water is 18.0 g/mol. MgSO4.5H20 a. O b. MgSO4.7H20 O c. MgSO4:3H20 d. MgSO4:H20
When a 7.50 g sample of hydrated LiClO, is heated to drive off all the water, the anhydrous residue that remains has a mass of 4.97 g. What is the mass percent of water in the hydrate?
4. When a 7.50 g sample of hydrated LiClo, is heated to drive off all the water, the anhydrous residue that remains has a mass of 4.97 g. What is the mass percent of water in the hydrate?
5. A 1.547 g sample of CuSO, XH,O is heated to drive off the water leaving behind 0.989 g of anhydrous Cuso, What is the value of x for this hydrate?
1. A mass of 3.462 g of a metal carbonate, MCO3, is heated to drive off carbon dioxide. The remaining metal oxide has a mass of 2.229 g. MCO3(s) → MO(s) + CO2(g) What is the identity of the metal?
H20 MASS of H20 2.09 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula.
3. What happens when a hydrate is heated? 4. A hydrate of CoCl, with a mass of 6.00 g is heated strongly. After cooling, the mass of the anhydrate is 3.27 g. a. How many grams of H2O were lost from the hydrate? b. What is the % water in the hydrate? c. What is the formula of the CoCl, hydrate? d. Write the equation for the dehydration of the CoCl, hydrate.