Would the percent yield of Ni(NH3)nCl2 be high, lower, or unchanged if you made the following procedural changes?
a) You performed the synthesis reaction at 100 degrees instead of 60 degrees
b) you dissolved the NiCl2*6H2O in 50 mL of distilled water instead of 10mL
c) You did not wash the Ni(NH3)nCl2 crystals with concentrated NH3 solution before drying them.
a) Well, let's think about it. If you perform the synthesis reaction at 100 degrees instead of 60 degrees, it's like turning up the heat in the kitchen. So that means reactions would happen faster, right? Therefore, the percent yield would likely be lower because the reaction might not have enough time to fully complete before you reach your desired product. So, we're talking about a lower yield here, like getting a smaller slice of pizza when you're really hungry.
b) Ah, the power of dilution! If you dissolve the NiCl2*6H2O in 50 mL of distilled water instead of 10 mL, you're basically giving it more space to stretch its legs, like filling a bigger swimming pool. This means that the ions have more room to move around and collide with each other, potentially allowing for a higher percent yield. So, it's like having more slices of pizza at a party - there's a greater chance for everyone to get a piece!
c) Oh no, skipping the wash? That's like going straight from the gym to a fancy dinner without showering! Not washing the Ni(NH3)nCl2 crystals with concentrated NH3 solution before drying them could leave behind impurities, like leftover reactants or byproducts. These impurities might interfere with the drying process and affect the overall yield. So, in this case, the percent yield would likely be lower because you're letting some unwanted guests crash your product party.
a) If the synthesis reaction is performed at 100 degrees instead of 60 degrees, the percent yield of Ni(NH3)nCl2 may be affected. Higher temperatures can sometimes increase the reaction rate and favor product formation. However, different reaction conditions may also lead to side reactions or product decomposition, reducing the overall yield. Without specific information about the reaction kinetics and thermodynamics, it is difficult to determine whether the percent yield would be higher or lower. Therefore, the effect of the temperature change on the percent yield is uncertain.
b) If the NiCl2*6H2O is dissolved in 50 mL of distilled water instead of 10 mL, the percent yield of Ni(NH3)nCl2 may be higher or lower. The reaction rate and yield could be affected by the change in reactant concentration. If the increased volume of water is still within the stoichiometric proportions required for the reaction, it may not significantly impact the yield. However, if the excess water affects the reaction conversion, it could lead to a lower percent yield.
c) If the Ni(NH3)nCl2 crystals are not washed with concentrated NH3 solution before drying, the percent yield may be lower. The purpose of washing the crystals with NH3 solution is to remove impurities and byproducts from the reaction. If the crystals are not washed, the impurities may remain and contribute to a lower yield. Washing the product helps to ensure a purer sample, which can improve the percent yield.
To determine the impact of the procedural changes on the percent yield of Ni(NH3)nCl2, we need to understand the underlying principles of the reaction and the factors that can affect the yield.
a) Performing the synthesis reaction at a higher temperature (100 degrees instead of 60 degrees) can potentially increase the reaction rate. This is because higher temperatures generally provide more energy to the reactant molecules, increasing their chance of successful collisions and thereby increasing the rate of reaction. Therefore, by increasing the temperature, the reaction may proceed more quickly, leading to a higher percent yield of the desired product.
b) Dissolving the NiCl2ยท6H2O in a larger volume of water (50 mL instead of 10 mL) does not directly impact the percent yield. The amount of water used primarily affects the concentration of the reactants, which can influence the reaction rate but not necessarily the yield. However, it is important to note that a higher volume of water might require a longer time for complete reactions and subsequent product formation.
c) Washing the Ni(NH3)nCl2 crystals with concentrated ammonia (NH3) solution before drying is a step typically performed to remove impurities and unreacted starting materials. By not performing this wash, impurities might still be present in the crystals. Depending on the nature and quantity of the impurities, they might affect the yield in different ways. If the impurities are inert or do not interfere with the product formation, the percent yield might remain unchanged. However, if the impurities react or interfere with the product formation, the yield could be lower than expected.
Overall, a) increasing the reaction temperature might yield a higher percent yield of Ni(NH3)nCl2, b) increasing the volume of water doesn't directly impact the yield, and c) not washing the crystals might potentially lower the yield if impurities are present and interfere with product formation.
It is important to note that each reaction is unique, and the impact of procedural changes can vary. Experimental validation is necessary to determine the actual effects on the percent yield.