None, unless there is metallic potassium in the reaction mixture. Assuming excess potassium metal is present then 14 moles of KBr can be produced.
7BaBr2 + excess potassium -----> 14KBr + 7 Ba
14.17 mol BaBr2 has 2*14.17 mol Br in it, so 28.34 mol KBr can be produced (also 28.34 mol K is needed)
To find the number of moles in 22.23 g of KBr, we need to divide the given mass by the molar mass of KBr. The molar mass of KBr is 119 g/mol. Therefore, 22.23 g of KBr is equal to 0.187 moles.
To find the number of moles of KBr in the solution, first calculate the number of moles of KBr in the 25 mL solution using the given concentration and volume. $$moles = concentration \times volume$$ Then, multiply the moles by the molecular weight of KBr to get the mass of KBr in the solution if needed.
To find the number of moles of KBr in the solution, first convert the volume to liters (110mL = 0.110L). Then, use the formula: moles = molarity x volume in liters. So, moles of KBr = 0.290 mol/L x 0.110 L = 0.032 moles of KBr.
2 KBr + BaI2 ----> 2 KI + BaBr2
14.17 mol BaBr2 has 2*14.17 mol Br in it, so 28.34 mol KBr can be produced (also 28.34 mol K is needed)
14.17 mol BaBr2 has 2*14.17 mol Br in it, so 28.34 mol KBr can be produced (also 28.34 mol K is needed)
First write a balanced chemical equation: 2K + Br2 ---> 2KBR Find the limiting reactant by using the moles of each element and determining which one gives you the smallest number of moles of potassium bromide. 2.92 mol K (2 mol KBr/2 mol K)= 2.92 mol KBr 1.78 mol Br2 (2 mol KBR/1 mol Br2)=3.56 mol KBr potassium is your limiting reactant so the max. number of moles of KBr that can be produced is 2.92 mol of KBr
To find the number of moles in 22.23 g of KBr, we need to divide the given mass by the molar mass of KBr. The molar mass of KBr is 119 g/mol. Therefore, 22.23 g of KBr is equal to 0.187 moles.
To find the number of moles of KBr in the solution, first calculate the number of moles of KBr in the 25 mL solution using the given concentration and volume. $$moles = concentration \times volume$$ Then, multiply the moles by the molecular weight of KBr to get the mass of KBr in the solution if needed.
0.1868 moles
Unbalanced: KBr + BaI2 --> KI + BaBr2Balanced: 2KBr + BaI2 --> 2KI + BaBr2
To find the number of moles of KBr in the solution, first convert the volume to liters (110mL = 0.110L). Then, use the formula: moles = molarity x volume in liters. So, moles of KBr = 0.290 mol/L x 0.110 L = 0.032 moles of KBr.
2 KBr + BaI2 ----> 2 KI + BaBr2
The answer is 0,0509 mole.
To find the grams of KBr in the solution, first calculate the moles of KBr present by using the molarity formula: moles = Molarity x Volume (L). Then, convert moles of KBr to grams using its molar mass. For KBr, the molar mass is approximately 119 g/mol. Finally, perform the calculation to find the grams present in the solution.
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