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If the concentration of g of hno if it was dissolved in l of water is mol l what would

 
 

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4.In a simple reaction A ↔ A*, a molecule is interconvertible between two forms that differ in standard free energy ...

ard free energy G° by 18 kJ/mole, with A* having the higher G°. Use the table below to find how many more molecules will be in state A* compared with state A at equilibrium. If an enzyme lowered the activation energy of the reaction by 11.7 kJ/mole, how would the ratio of A to A* change? Table: RELATIONSHIP BETWEEN THE STANDARD FREE- ENERGY CHANGE, ∆G°, AND THE EQUILIBRIUM CONSTANT Hint: ∆G° represents the free-energy difference under standard conditions (where all components are present at a concentration of 1 mole/litter). From this table, we see that if there is a favourable free-energy change of –17.8 kJ/mole for the transition Y→ X, there will be 1000 times more molecules of X than of Y at equilibrium (K = 1000).
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5.If the concentration of 2.000g of HNO3 if it was dissolved in 2.000L of water is 0.01587 mol/L, What would ...

at would have been the concentration of HNO3 AFTER the 0.1000g of Li was added and allowed to react with some of HNO3? (Hint - Lim XS Problem) What would have been the pH of your acid solution after the metal was added?
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6.What would be the concentration of 2.000g of HNO3 if it was dissolved in 2.000L of water in moles per ...

r litre? What would have been the concentration of HNO3 AFTER the 0.1000g of Li was added and allowed to react with some of HNO3? (Hint - Lim XS Problem) What would have been the pH of your acid solution after the metal was added? If you wanted to fill a rubber balloon to an internal volume of 5.000L and pressure of 140.0kPa in a 25.00C room with hydrogen gas from the reaction of your metal and acid (Li and HNO3), what is the minimum quantity in millilitres of an 8.000M solution of your acid you would need to generate enough hydrogen gas? (assume you have more than enough metal).
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7.What would be the concentration of 2.000g of your acid if it was dissolved in 2.000L of water in moles ...

es per litre? What would be the pH of the above solution? What would have been the concentration of your acid AFTER the 0.1000g of your metal was added and allowed to react with some of your acid? (Hint - Lim/excess Problem)
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8.For the follwing reaction; 2A(g) B(g) + C(g) Kc is 0.640 at 348 K. If an initial concentration of 0.962 M ...

0.962 M compound A is allowed to equilibrate, what is the equilibrium concentration of compound C in molarity? Do not include unit. Keep 3 decimal places in your answer.
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1.AU MAT 120 Systems of Linear Equations and Inequalities Discussion

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